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26 September, 06:10

How many grams of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg (s) ? Show all calculations leading to an answer. List 3 indicators of a chemical change.

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  1. 26 September, 06:12
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    Balanced chemical reaction happening here is:

    3Mg (s) + N₂ (g) → Mg₃N₂ (s)

    moles of product formed from each reactant:

    2.0 mol of N2 (g) x 1 mol Mg₃N₂ = 2 mol Mg₃N₂

    1 mol N2

    and

    8.0 mol of Mg (s) x 1 mol Mg₃N₂ = 2.67 mol Mg₃N₂

    3 mol Mg

    Since N2 is giving the least amount of product (Mg₃N₂) ie. 2 mol Mg₃N₂

    N2 is the limiting reactant here and Mg is excess reactant.

    Hence mole of product formed here is 2 mol Mg₃N₂

    molar mass of Mg₃N₂

    = 3 Mg + 2 N

    = 101g/mol

    mass of product (Mg₃N₂) formed

    = moles x Molar mass

    = 2 x 101

    = 202g Mg₃N₂

    202g of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg (s).

    The following are indicators of chemical changes:

    Change in Temperature

    Change in Color

    Formation of a Precipitate
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